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Accelerated chemistry Part 2 midterm exam review

Total questions: 177

Worksheet time: 3hrs 26mins

Name
Class
Date
1.
What is the electron configuration of oxygen (O)?
a)
1s² 2s² 2p⁴
b)
1s² 2s² 2p²
c)
1s² 2s² 2p³
d)
1s² 2s² 2p⁵
2.
Which element has the electron configuration [Kr] 5s² 4d¹⁰ 5p⁵?
a)
Iodine (I)
b)
Astatine (At)
c)
Bromine (Br)
d)
Xenon (Xe)
3.
What is the maximum number of electrons that can occupy the n=3 shell?
a)
18.0
b)
8.0
c)
32.0
d)
2.0
4.
Which of the following represents an incorrect electron configuration?
a)
1s² 2s²
b)
1s² 2s² 2p⁶
c)
1s² 2s² 3p⁶
d)

1s² 2s² 2p⁵

5.
For the element with atomic number 11 (sodium), what is its electron configuration?
a)
1s² 2s² 2p⁶ 3s¹
b)
1s² 2s² 2p⁶ 3p¹
c)
1s² 2s² 3s²
d)
1s² 2s¹ 2p⁶ 3s¹
6.
What is the electron configuration for the element with atomic number 26 (iron)?
a)
[Ar] 4s² 3d⁶
b)
[Ar] 3s² 3p⁶ 3d⁶
c)
[Kr] 5s² 4d⁶
d)
[Ne] 3s² 3p⁶ 4s²
7.
According to the Aufbau principle, which orbital is filled after 4s?
a)
3d
b)
4p
c)
4s
d)
5s
8.
What is Hund's rule?
a)
Electrons fill orbitals singly before pairing
b)
Electrons fill from low to high energy
c)
Electrons occupy the lowest energy level first
d)
Orbitals cannot hold more than two electrons
9.
How many electrons can a single orbital hold?
a)
2.0
b)
6.0
c)
8.0
d)
4.0
10.
Which of the following is the correct order of filling for the d-block elements?
a)
3d, 4s, 4p
b)
4p, 4s, 3d
c)
3p, 4s, 3d
11.
What is the electron configuration for the element with atomic number 17 (chlorine)?
a)
[Ne] 3s² 3p⁵
b)
[Ar] 3s² 3p³
c)
[Ne] 3p⁶
d)
[Ne] 3s² 3p⁶
12.
In which subshell does the last electron enter for the element with atomic number 29 (copper)?
a)
4s
b)
3d
c)
4p
d)
5s
13.
What is the maximum number of electrons in the n=4 shell?
a)
32.0
b)
18.0
c)
8.0
d)
2.0
14.

Part A of an electron configuration is:

a)

Principal energy level

b)

Subshell

c)

Number of electrons

d)

Number of protons

15.

Part B of an electron configuration is:

a)

Principal energy level

b)

Subshell

c)

Number of electrons

d)

Number of protons

16.

Part C of an electron configuration is:

a)

Principal energy level

b)

Subshell

c)

Number of electrons

d)

Number of protons

17.

The image shows the partial electron configuration of manganese (Mn). Below there are two empty boxes. Correctly drag the final two answers in the correct order to finish its electron configuration.​

​ ​ (a)   ​ (b)  

Choose from the below words
4s²
3d⁵
1p⁶
2s³
3d⁹
2d⁹
18.

What is the maximum number of electrons that an S orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

19.

How many electrons can the d sublevel(orbital) hold?

a)

8

b)

10

c)

2

d)

4

20.

There are 4 different types of subshells(orbitals) s,p,d,f

a)

true

b)

false

21.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

22.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
23.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
24.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
25.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
26.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

27.

What is the electron configuration for an oxide ion (O²⁻)?

a)

1s² 2s² 2p⁴

b)

1s² 2s² 2p⁶

c)

1s² 2s² 2p³

d)

1s² 2s² 2p⁵

28.

Which of the following represents the correct electron configuration for a magnesium ion (Mg²⁺)?

a)

1s² 2s² 2p⁶ 3s²

b)

1s² 2s² 2p⁶

c)

1s² 2s² 2p⁶ 3s² 3p⁶

d)

1s² 2s² 2p⁶ 3p²

29.

What is the electron configuration of a chloride ion (Cl-)?

a)
1s² 2s² 2p⁶ 3s² 3p⁷
b)
1s² 2s² 2p⁶ 3s² 3p⁴
c)
1s² 2s² 2p⁶ 3s² 3p⁵
d)
1s² 2s² 2p⁶ 3s² 3p⁶
30.

How many VALENCE ELECTRONS does Chlorine have?

a)

2

b)

7

c)

8

d)

10

e)

17

31.

Ionic bonds are formed when electrons get

a)

Shared between two atoms

b)

Removed from both atoms

c)

Transferred from one atom to another

d)

Added to both atoms

32.

Ionic bonds typically form between

a)

A metal and a nonmetal

b)

Two nonmetals

c)

Two metals

d)

A metalloid and a metal

33.

What is the correct formula for Sodium Chloride?

a)

SCl

b)

NaCl

c)

SC

d)

NaCl2

34.

Name this ionic compound: Al2O3

a)

Dialuminum oxide

b)

Aluminum oxygen

c)

Oxygen Aluminide

d)

Aluminum oxide

35.

Cations _______ electrons, becoming _______ charged.

a)

Gain; positively (+)

b)

Gain; negatively (-)

c)

Lose; positively (+)

d)

Lose; negatively (-)

36.

Anions ____ electrons, becoming _____ charged.

a)

Gain; positively (+)

b)

Gain; negatively (-)

c)

Lose; positively (+)

d)

Lose; negatively (-)

37.

Write the chemical formula for a compound formed by K and Br (potassium bromide).

a)

KBr

b)

K2Br

c)

KBr3

d)

KBr2

38.

Metals (like Na) typically _____ electrons in the formation of ionic bonds.

a)

Gain

b)

Lose

c)

Keep the same

39.

Nonmetals (like Cl) typically ____ electrons when they form ionic bonds.

a)

Gain

b)

Lose

c)

Keep the same

40.

Using the model for the formation of Scandium Fluoride (an ionic compound), can you guess its chemical formula?

a)

Sc3F

b)

Sc3F3

c)

Sc+3F-1

d)

ScF3

41.

In formation of ionic compounds, the electrons from a particular atom are transferred so that the atom can attain stable configuration of a noble element. What noble configuration does Sodium ion attain?

a)

Hellium

b)

Neon

c)

Argon

d)

Krypton

42.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

43.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

44.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

45.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

46.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium II sulfate

d)

cesium II sulfide

47.

When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..

a)

atomic number

b)

mass number

c)

charge

d)

ionization energy

48.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

49.

When naming a compound, what must the last part be?

a)

the element with "ide" at the end

b)

the element with the ending "ite"

c)

the name of the element

d)

the element with "ide" at the end, unless its a polyatomic ion

50.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

51.

What is the name of the compound Sc(OH)3?

a)

Scandium (III) hydroxide

b)

Scandium (I) hydroxide

c)

Scandium (II) hydroxide

d)

Scandium hydroxide

52.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

53.

By looking at the formula of an ionic compound, we can determine the charge (oxidation state) of a transition metal.

a)

True

b)

False

54.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

55.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

56.

NH4OH

a)

nitrogen hydrogen oxide hydride

b)

ammonium hydroxide

c)

ammonia hydride

d)

ammonium oxide

57.

What is the charge of Cobalt (III)

a)

3+

b)

2+

c)

8+

d)

3-

58.

What is the correct formula for Aluminum Suflite

a)

Al2SO4

b)

Al2SO3

c)

Al2(SO4)3

d)

Al2(SO3)3

59.

What is the name for NaHCO3

a)

Sodium Bicarbonate

b)

Sodium Carbonate

c)

Sodium Hydrogen Chloride

d)

Sodium

Hypochlorite

60.

a chemical bond that results from the sharing of valence electrons

a)

covalent bond

b)

pi bond

c)

sigma bond

d)

coordinate covalent bond

61.

a model that uses electron-dot structures to show how electrons are arranged in molecules. Pairs of dots or lines represent bonding pairs

a)

resonance

b)

Lewis structure

c)

structural formula

d)

molecule

62.

Valence Shell Electron Pair Repulsion model, which is based on an arrangement that minimizes the repulsion of shared and unshared pairs of electrons around the central atom

a)

VSPER model

b)

resonanace

c)

lewis structure

d)

structural formula

63.

A type of bond that forms when electrons are not shared equally.

a)

coordinate covalent bond

b)

polar covalent bond

c)

covalent bond

d)

oxyacid

64.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
65.

What is it called if there are three-pairs of electrons being shared between two atoms?

a)

Triple bond

b)

Bond length

c)

Tribond

d)

Chocolate Mousse

66.
How many electrons should Carbon have around its Lewis dot structure?
a)
1
b)
3
c)
4
d)
5
67.

What types of atoms make a covalent bond?

a)

2 Nonmetals

b)

1 Nonmetal & 1 Metal

c)

2 Metals

d)

2 Noble Gases

68.
What is a diatomic element?
a)
a metal bonded with a nonmetal
b)
2 or more nonmetals bonded together
c)
2 or more metals bonded together
d)
2 atoms of the same element bonded together
69.
The number of bonds an element will form in a covalent compound will be equal to
a)
the number of valence electrons
b)
eight electrons
c)
the number of electrons needed to reach an octet
d)
the group number
70.
The desire for an element to have 8 atoms around it is called 
a)
Octet Rule
b)
Resonance
c)
Ionization energy
d)
Electronegativity
71.

How many Valence Electrons does Oxygen have?

a)

2

b)

7

c)

6

d)

1

72.

Which of the following elements will make 3 covalent bonds?

a)

Oxygen

b)

Phosphorous

c)

Fluorine

d)

Germanium

73.
Which of the following is a Diatomic Molecule 
a)
K2
b)
C2
c)
S2
d)
N2
74.
What is the name of this Molecule shape
a)
Tetrahedral
b)
Trigonal Pyramidal 
c)
Trigonal bipyramidal
d)
Bent
75.
Which of these would be covalently bonded
a)
Fr and K
b)
Sc and O 
c)
F and Cl
d)
He and Pt
76.

What shape would this have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

77.

What is the shape of a water molecule?

a)
tetrahedral structure
b)
linear structure
c)
trigonal planar structure
d)
bent structure
78.

Because electron pairs repel, molecules adjust their shapes so that the valence electron pairs are as far apart as possible.

a)

structural formula

b)

VSEPR theory

c)

resonance structures

d)

polar molecules

79.

Atoms form bonds in order to have an electron configuration similar to a ___________.

a)

noble gas

b)

alkali metal

c)

friend

d)

neighbor

80.

The element nitrogen (N) has ___ valence electrons and needs ___ electrons to complete its octet.

a)

5 , 3

b)

3 , 5

c)

6 , 2

d)

2 , 6

81.

What type of chemical bond is being shown in the F2 molecule?

a)

single covalent bond

b)

double covalent bond

c)

triple covalent bond

d)

quadruple covalent bond

82.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

83.

What is the bond angle in a bent molecule with four things around the central atom? 

a)

120

b)

<109.5

c)

109.5

d)

180

84.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
85.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

86.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

87.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

88.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

89.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
90.
What geometry will this molecular structure have?: CCl4
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
91.

What is the molecular geometry for this molecule?

a)

Bent

b)

Trigonal pyramidal

c)

Trigonal planar

d)

Linear

92.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
93.

Determine the molecular geometry of the given structure.

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Trigonal Planar

d)

Tetrahedral

94.
*
a)
linear
b)
trigonal planar
c)
trigonal pyramid
d)
bent of angular
95.
*
a)
trigonal pyramid
b)
linear
c)
bent
d)
angular
96.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
97.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
98.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
99.
What is the chemical formula for Phosphorus Pentachloride?
a)
PCl
b)
PCl3
c)
PCl5
d)
P5Cl
100.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
101.
H2S has what kind of intermolecular force?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
102.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
103.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
104.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

105.

Which intermolecular force requires hydrogen and one of the following: nitrogen, oxygen, fluorine?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

106.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

107.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

108.

Rank these in order of strength:
London forces
hydrogen bond
dipole-dipole attraction

a)

dipole-dipole> hydrogen bond> London

b)

London> dipole-dipole> hydrogen bond

c)

hydrogen bond> dipole-dipole> London

d)

hydrogen bond> dipole-dipole> London

109.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)
1
b)
2
c)
3
d)
4
110.

Which equation is balanced?

a)

PbO2 + 2H2

b)

SO2 + H20 --> H2SO4

c)

2Na + 2H2O --> 2NaOH + H2

111.

Balance this equation

_Al +_HCl --> _H2 +_AlCl3

a)

2,6,3,2

b)

it's already balanced

c)

4,12,3,4

d)

2,1,4,5

112.

What are the coefficients that would properly balance this equation?

__Ca + __H2O --> __Ca(OH)2 + __H2

a)

2,1 --> 2,1

b)

1,2 --> 1,1

c)

1,2 --> 2,4

d)

1,2 --> 2,1

113.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__CO + __Fe2O3--> __Fe + __CO2
a)
3,1 --> 2,3
b)
3,2 --> 1,1
c)
3,2 --> 2,4
d)
3,2 --> 2,1
114.

What are the coefficients that would properly balance this equation?

__AgNO3 + __H2S --> __Ag2S+ __HNO3

a)

2,1 --> 1,2

b)

1,2 --> 1,1

c)

1,2 --> 1,2

d)

1,2 --> 2,1

115.

What are the coefficients that would properly balance this equation?

__H2 + __S --> __H2S

a)

1,1 --> 1

b)

2,2 --> 2

c)

1,2 --> 1

d)

1,2 --> 2

116.

What are the coefficients that would properly balance this equation?

__Al + __O2--> __Al2O3

a)

4,1 --> 2

b)

4,3 --> 4

c)

3,4 --> 1

d)

4,3 --> 2

117.

Determine the coefficients to make the following equation balanced?

__N2 + __O2--> __NO

a)

1, 1, 1

b)

1, 1, 2

c)

2, 2, 2

d)

1, 2, 2

118.

Determine the coefficients to balance the equation.

__Al +__HCl --> __H2 +__AlCl3

a)

2,6,3,2

b)

it's already balanced

c)

4,12,3,4

d)

2,1,4,5

119.

Balance the the following equation.

__Zn+__HCl -->__ZnCl2 +__H2

a)

1,1,2,1

b)

1,1,1,2

c)

1,2,1,1

d)

2,1,1,1

120.

What type of reaction is the equation C + O2 → CO2?

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

121.

What type of reaction is the equation


2NaCl → 2Na + Cl2?

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

122.

What type of reaction is the equation

Cu + 2Ag(NO3) → 2Ag + Cu(NO3)

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

123.

What type of reaction is the equation


MgCl2 + Li2CO3 → MgCO3 + 2 LiCl

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

124.

What type of reaction is the equation


3Pb + 2H3PO4 → 3H2 + 1Pb3(PO4)2

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

125.

What type of reaction is the equation

3 HBr + 1 Al(OH)3 → 3 H­2O + 1 AlBr3

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

126.

What type of reaction is the equation

2 RbNO3 + BeF2 → Be(NO3)2 + 2 RbF

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

127.

What type of reaction is the equation

P4 + 3 O2 → 2 P2O3

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

128.

What equation has the following general formula:

AB → A + B

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

e)

Combustion

129.

What equation has the following general formula:

AB + CD → CB + AD

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

e)

Combustion

130.

What equation has the following general formula:
CxHy + O2 →  CO2 + H2O  + EC_xH_y\ +\ O_2\ \rightarrow\ \ CO_{2\ }+\ H_2O\ \ +\ E  

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

e)

Combustion

131.

What type of equation is shown by the following:
C11H24+17O2  →  11CO2 + 12H2O + EC_{11}H_{24}+17O_2\ \ \rightarrow\ \ 11CO_2\ +\ 12H_2O\ +\ E  

a)

Synthesis

b)

Decomposition

c)

Single Displacement

d)

Double Displacement

e)

Combustion

132.
Fill in the blanks with coefficient:
PCl5+_ H2O→_ HCl+H3PO4
a)
4, 5
b)
1, 6
c)
3, 8
d)
2,2
133.
Balance this equation
_Zn+_HCl-->_ZnCl2 +_H2
a)
1,1,2,1
b)
1,1,1,2
c)
1,2,1,1
d)
2,1,1,1
134.
Balance this equation.
_Mg + _Cl2 --> _MgCl2
a)
1, 2,1
b)
already balanced
c)
2,1,1
d)
1,1,2
135.
Balance this equation
_N2 + _H2 --> _NH3
a)
1,2,3
b)
1,3,2
c)
1,1,2
d)
2,1,1
136.

What type of reaction is the equation


2NaCl → 2Na + Cl2?

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

137.

What type of reaction is the equation

Cu + 2Ag(NO3) → 2Ag + Cu(NO3)

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

138.

What type of reaction is the equation


MgCl2 + Li2CO3 → MgCO3 + 2 LiCl

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

139.
When balancing equations a ____ can be placed to the left of a formula of a substance to make the equations balanced
a)
charge
b)
subscript
c)
random number
d)
coefficient
140.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction. 
141.
What is the little number after an element in a chemical equation called.
Example: H2
a)
Coefficient 
b)
Subscript
c)
Atom
d)
Equation
142.
Balance this equation.
_CF4 + _Br2 -- _CBr4 + _F2
a)
2,1,2,1
b)
1,2,2,1
c)
1,2,1,2
d)
2,2,2,2
143.
Which problem is balanced?
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
144.

Identify the type of reaction:

ZnCl2 + Mg --> Zn + MgCl2

a)

Precipitate

b)

Single Replacement

c)

Double Replacement

d)

Decomposition

145.

Identify the reaction type for the following equation:

K + F2 --> KF

a)

Double replacement

b)

Single Replacement

c)

Synthesis

d)

Decomposition

146.

Identify the reaction type:

C2H6 + O2 --> CO2 + H2O

a)

Double replacement

b)

Synthesis

c)

Acid base

d)

Combustion

147.

What is the type of reaction shown above?

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

148.
One reactant into several products.
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
149.
Two Reactants and One Product
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
150.
Balance this equation
_Zn+_HCl-->_ZnCl2 +_H2
a)
1,1,2,1
b)
1,1,1,2
c)
1,2,1,1
d)
2,1,1,1
151.
When balancing equations a ____ can be placed to the left of a formula of a substance to make the equations balanced
a)
charge
b)
subscript
c)
random number
d)
coefficient
152.

Which side of a chemical equation is the product side?

a)
Left (before the yields sign)
b)
Right (after the yields sign)
153.
Which side of a chemical equation is the reactant side?
a)
Left (before the yields sign)
b)
Right (after the yields sign)
154.
The Law of Conservation of Matter states that the total mass of the reactants should be 
a)
More than the mass of the products
b)
Equal to the mass of the products
c)
Ignored during the reaction
d)
Less than the mass of the products
155.
What are Chemical Reactions?
a)
It's when you mix substances.
b)
a process in which atoms rearrange to form new substances
c)
When something bubbles.
d)
letter and numbers showing the types and number of atoms
156.
the starting materials in a chemical reaction
a)
Products
b)
Reactants
c)
Starters
d)
Enders
157.
a substance that is formed as the result of a chemical reaction
a)
Product 
b)
Reactant
c)
Starters
d)
Enders
158.
AB + CD →AD + CB
a)
Double Replacement
b)
Single Replacement
c)
Synthesis
d)
Decomposition
159.

What mathematical function do coefficients perform in a balanced equation?

a)

addition

b)

multiplication

c)

subtraction

d)

division

160.

Which of the following is an example of a synthesis reaction?

a)
b)
c)
d)
161.

Which of the following is an example of a decomposition reaction?

a)
b)
c)
d)
162.

Which of the following is an example of a single replacement reaction?

a)
b)
c)
d)
163.

Which of the following is an example of a double replacement reaction?

a)
b)
c)
d)
164.

The red numbers in the image represent

a)

subscripts

b)

coeffiecients

c)

roman numerals

d)

none of the answer options are correct

165.

The blue numbers in the image represent

a)

subscripts

b)

coeffiecients

c)

roman numerals

d)

none of the answer options are correct

166.
Which problem is balanced?
(Check ALL answers)
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
167.
Is this balanced?
Al + O2 → 2Al2O3
a)
Yes
b)
No
168.

Balance this reaction:

____ Na3PO4 + ____ KOH ---> ____ NaOH + ____ K3PO4

a)

1,3,3,1

b)

1,3,2,1

c)

2,3,3,1

d)

1,1,3,1

169.

Which type of reaction is:

2 H3AsO4 → As2O5 + 3 H2O

a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Combustion
170.
Which type of reaction is: C2H4 + 3 O2 → 2 CO2 + 2 H2O
a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Combustion
171.

Which type of reaction is:

2 NaBr + Ca(OH)2 → CaBr2 + 2 NaOH

a)
Synthesis
b)
Single Displacement
c)
Double Displacement
d)
Combustion
172.

Balance the following:

____ H2SO4 + ____ NaNO2 → ____ HNO2 + ____ Na2SO4

a)
1,1,2,1
b)
1,2,2,1
c)
2,3,3,2
d)
4,3,2,1
173.

In the equation, 2Mg + O2 ---> 2MgO, which are the reactants?

a)

Mg and O2

b)

MgO

c)

Mg and MgO

d)

O and MgO

174.

Balance this equation:

​ (a)   Fe + ​ (b)   O2 --> ​ (c)   Fe2O3

Choose from the below words
4
3
2
1
0
175.

What are the coefficients that would properly balance this equation?

__C3H8 + __O2 --> __CO2 + __H2O

a)

2, 7 --> 6, 8

b)

1, 5 --> 3, 4

c)

2, 5 --> 4, 6

d)

1, 4 --> 2, 3

176.

Identify the type of reaction:

2Na + Cl2 --> 2NaCl

a)

Single Replacement

b)

Double replacement

c)

Synthesis

d)

Decomposition

177.

Determine the coefficients to balance the equation.

__Fe + __O2 --> __Fe2O3

a)

1, 1 --> 1

b)

2, 1 --> 1

c)

4, 3 --> 2

d)

3, 2 --> 1

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